A 0.1475-M solution of Ba(OH)2 was used to titrate the acetic acid (60.05 g/mol) in a dilute aqueous solution. The following results were obtained. (See attached image) (a) Calculate the mean w/v percentage of acetic acid in the sample. (b) Calculate the standard deviation for the results. (Take note if n-1 should be used) (c) Calculate the 90% confidence interval for the mean. (d) (d) At the 90% confidence level, could any of the results be discarded?
A 0.1475-M solution of Ba(OH)2 was used to titrate the acetic acid (60.05 g/mol) in a dilute aqueous solution. The following results were obtained. (See attached image) (a) Calculate the mean w/v percentage of acetic acid in the sample. (b) Calculate the standard deviation for the results. (Take note if n-1 should be used) (c) Calculate the 90% confidence interval for the mean. (d) (d) At the 90% confidence level, could any of the results be discarded?
Chemistry for Engineering Students
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ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter3: Molecules, Moles, And Chemical Equations
Section: Chapter Questions
Problem 3.37PAE: 3.37 If atypical grain of sand occupies a volume of 1.3 × 10-4 cm3, what is the volume (in cm3) of 1...
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A 0.1475-M solution of Ba(OH)2 was used to titrate the acetic acid (60.05 g/mol) in a dilute aqueous solution. The following results were obtained. (See attached image)
(a) Calculate the mean w/v percentage of acetic acid in the sample.
(b) Calculate the standard deviation for the results. (Take note if n-1 should be used)
(c) Calculate the 90% confidence interval for the mean.
(d) (d) At the 90% confidence level, could any of the results be discarded?
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